Liquids $A$ and $B$ form an ideal solution. The vapour pressure of pure $A$ and $B$ are $50 \ mm \ Hg$ and $32 \ mm \ Hg$ respectively at $300 \ K$. One mole of liquid $A$ is mixed with $1$ mole of liquid $B$. What is the approximate mole fraction of $A$ in the vapour phase?

Total vapour pressure of a mixture of $1 \, mol \, X$ $(P_x^o = 150 \, torr)$ and $2 \, mol \, Y$ $(P_y^o = 300 \, torr)$ is $240 \, torr$. In this case:

When $25 \ mL$ of acetone is mixed with $25 \ mL$ of ethanol,the volume of the resulting solution will be ...........

Two liquids $A$ and $B$ form an ideal solution at temperature $T \ K$. At $T \ K$,the vapour pressures of pure $A$ and $B$ are $55 \ kNm^{-2}$ and $15 \ kNm^{-2}$ respectively. What is the mole fraction of $A$ in the solution of $A$ and $B$ in equilibrium with a vapour in which the mole fraction of $A$ is $0.8$?

Identify the mixture that shows positive deviations from Raoult's Law.

In a mixture of $A$ and $B$ components,the solution shows positive deviation from Raoult's law when: